covalent bond/ molecular geometry

octet rule exceptions

1. The third row and lower can exceed the octet rule

2. H only 2, Be only 4, B and Al only (usually)

3. molecules with odd number of electrons

ED: 2 UE: 0

hybridization: sp

bond angle: 180

electron domain geometry: Linear

molecular geometry: Linear

ED: 3 UE: 0

hybridization: sp²

bond angle: 120

electron domain geometry: trigonal planar

molecular geometry: trigonal planar

ED: 3 UE: 1

hybridization: sp²

bond angle: 120

electron domain geometry: trigonal planar

molecular geometry: bent

ED: 4 UE: 0

hybridization: sp³

bond angle: 109.5

electron domain geometry: Tetrahedral

molecular geometry: Tetrahedral

ED: 4 UE: 1

hybridization: sp³

bond angle: 109.5

electron domain geometry: Tetrahedral

molecular geometry: trigonal pyramidal

ED: 4 UE: 2

hybridization: sp³

bond angle: 109.5

electron domain geometry: Tetrahedral

molecular geometry: bent

ED: 5 UE: 0

hybridization: sp³d

bond angle: 90, 120

electron domain geometry: Trigonal bipyramidal

molecular geometry: trigonal bipyramidal

ED: 5 UE: 1

hybridization: sp³d

bond angle: 90, 120

electron domain geometry: Trigonal bipyramidal

molecular geometry: See-Saw

ED: 5 UE: 2

Hybridization: sp³d

bond angle: 90, 120

electron domain geometry: Trigonal bipyramidal

molecular geometry: T-shaped

ED: 5 UE: 3

Hybridization: sp³d

bond angle: 90, 120

electron domain geometry: Trigonal bipyramidal

molecular geometry: linear

ED: 6 UE: 0

Hybridization: sp³d²

bond angle: 90

electron domain geometry: Octahedral

molecular geometry: octahedral

ED: 6 UE: 1

Hybridization: sp³d²

bond angle: 90

electron domain geometry: Octahedral

molecular geometry: square pyramidal

ED: 6 UE: 2

Hybridization: sp³d²

bond angle: 90

electron domain geometry: Octahedral

molecular geometry: square planar

sigma and pi bonds

one sigma bond in each bond

alkali metals

low ionization energies, highly reactive in water, readily form ionic compounds

alkaline earth metals

lower ionization energies, most are reactive with water

halogens

high electron affinities/electronegativities, highly reactive with metals; good oxidizing agents

noble gases

inert gases (full octet)

transition metals

often form colored compounds